Ionisation energy of ' K ' would be same as : | TestHub

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Amount of energy required to remove the most loosely bonded electron from an isolated gaseous atom from its ground state electronic configuration is called ionization energy. The value of ionization energy mainly depends on (i) $Z_{e ff}$ , (ii) atomic radius, and (iii) the screening effect of inner electrons. Successive ionization energies of an element always follow an increasing order.

Ionisation energy of ' K ' would be same as :

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Answer:

A

Solution:

The ionization energy of K is the energy required to remove an electron from a neutral K atom: $K (g) \to K^{+} (g) + e^{-}$ . This is the reverse process of the electron affinity of $K^{+}$ , which is $K^{+} (g) + e^{-} \to K (g)$ . By definition, the energy change for a forward reaction is equal in magnitude but opposite in sign to the reverse reaction. Therefore, the ionization energy of K is equal to the electron affinity of $K^{+}$ .

Stream:JEESubject:ChemistryTopic:PERIODIC TABLESubtopic:Ionisation Energy,

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